1. This question is about modelling the thermal processes involved when a person is running.

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1 1. This question is about modelling the thermal processes involved when a person is running. When running, a person generates thermal energy but maintains approximately constant temperature. (a) Explain what thermal energy and temperature mean. Distinguish between the two concepts (4) The following simple model may be used to estimate the rise in temperature of a runner assuming no thermal energy is lost. A closed container holds 70 kg of water, representing the mass of the runner. The water is heated at a rate of 1200 W for 30 minutes. This represents the energy generation in the runner. (b) (i) Show that the thermal energy generated by the heater is J. (ii) Calculate the temperature rise of the water, assuming no energy losses from the water. The specific heat capacity of water is 4200 J kg 1 K 1. 1

2 (c) The temperature rise calculated in (b) would be dangerous for the runner. Outline three mechanisms, other than evaporation, by which the container in the model would transfer energy to its surroundings (6) A further process by which energy is lost from the runner is the evaporation of sweat. (d) (i) Describe, in terms of molecular behaviour, why evaporation causes cooling. 2

3 (ii) Percentage of generated energy lost by sweating: 50% Specific latent heat of vaporization of sweat: J kg 1 Using the information above, and your answer to (b) (i), estimate the mass of sweat evaporated from the runner. (iii) State and explain two factors that affect the rate of evaporation of sweat from the skin of the runner. (4) (Total 25 marks) 2. This question is about an experiment to measure the temperature of a flame. (a) Define heat (thermal) capacity (1) 3

4 A piece of metal is held in the flame of a Bunsen burner for several minutes. The metal is then quickly transferred to a known mass of water contained in a calorimeter. flame water calorimeter container Bunsen burner lagging (insulation) The water into which the metal has been placed is stirred until it reaches a steady temperature. (b) Explain why (i) the metal is transferred as quickly as possible from the flame to the water; (1) (ii) the water is stirred. (1) The following data are available: heat capacity of metal = 82.7 J K 1 heat capacity of the water in the calorimeter = J K 1 heat capacity of the calorimeter = 54.6 J K 1 initial temperature of the water = 288 K final temperature of the water = 353 K 4

5 (c) Assuming negligible energy losses in the processes involved, use the data to calculate the temperature T of the Bunsen flame (4) (Total 7 marks) 3. This question is about thermal physics. (a) Explain why, when a liquid evaporates, the liquid cools unless thermal energy is supplied to it (b) State two factors that cause an increase in the rate of evaporation of a liquid

6 (c) Some data for ice and for water are given below. Specific heat capacity of ice = J kg 1 K 1 Specific heat capacity of water = J kg 1 K 1 Specific latent heat of fusion of ice = J kg 1 A mass of 350 g of water at a temperature of 25 C is placed in a refrigerator that extracts thermal energy from the water at a rate of 86 W. Calculate the time taken for the water to become ice at 5.0 C (4) (Total 9 marks) 4. Temperature and thermal energy (a) Outline how a temperature scale is constructed (b) Discuss why even an accurate thermometer may affect the reliability of a temperature reading

7 (c) (i) Define specific heat capacity. (ii) The table below gives data for water and ice. specific heat capacity of water specific latent heat of fusion of ice 4.2 kj kg 1 K kj kg 1 A beaker contains 450 g of water at a temperature of 24 C. The thermal (heat) capacity of the beaker is negligible and no heat is gained by, or lost to, the atmosphere. Calculate the mass of ice, initially at 0 C, that must be mixed with the water so that the final temperature of the contents of the beaker is 8.0 C. (4) 7

8 (d) (i) Distinguish between evaporation and boiling. (ii) Explain, in terms of molecular behaviour, why boiling involves a transfer of thermal energy with no change in temperature. (Total 15 marks) 8

9 5. This question is about the change of phase (state) of ice. A quantity of crushed ice is removed from a freezer and placed in a calorimeter. Thermal energy is supplied to the ice at a constant rate. To ensure that all the ice is at the same temperature, it is continually stirred. The temperature of the contents of the calorimeter is recorded every 15 seconds. The graph below shows the variation with time t of the temperature θ of the contents of the calorimeter. (Uncertainties in the measured quantities are not shown.) / C t / s (a) (b) On the graph above, mark with an X, the data point on the graph at which all the ice has just melted. Explain, with reference to the energy of the molecules, the constant temperature region of the graph (1) 9

10 The mass of the ice is 0.25 kg and the specific heat capacity of water is 4200 J kg 1 K 1. (c) Use these data and data from the graph to (i) deduce that energy is supplied to the ice at the rate of about 530 W. (ii) determine the specific heat capacity of ice. (iii) determine the specific latent heat of fusion of ice. (Total 12 marks) 10

11 6. The physics of cooling (a) Explain what is meant by the temperature of a substance A thermometer is placed in a liquid contained in an open beaker. The reading of the thermometer is recorded at regular intervals. The variation with time t of the temperature θ is shown below. / C (b) t / s The temperature of the surroundings is 20 C. On the graph continue the line to show the variation with time of the temperature for the next 3000 s. (c) By reference to the graph, state and explain the rate of loss of thermal energy from the substance between (i) 0 and 600 s; 11

12 (ii) 600 and 1800 s. (4) The mass of the liquid is 0.11 kg and the specific heat capacity of the liquid is 1300 J kg 1 K 1. (d) (i) Use the graph to deduce that the rate of loss of thermal energy at time t = 600 s is approximately 4 W. (ii) Calculate the specific latent heat of fusion of the liquid. (Total 16 marks) 12

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